Fe2(SO4)3 + 3Ca(OH)2 → 3CaSO4 + 2Fe(OH)3
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The reaction of iron(III) sulfate and calcium hydroxide yields calcium sulfate and iron(III) hydroxide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of iron(III) sulfate and calcium hydroxide
General equation
- Reaction of salt of weak base and strong base
- Salt of weak baseBrønsted acid + Strong baseBrønsted base ⟶ Salt of strong baseConjugate acid + Weak baseConjugate base + (H2O)
Oxidation state of each atom
- Reaction of iron(III) sulfate and calcium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe2(SO4)3 | Iron(III) sulfate | 1 | Brønsted acid | Salt of weak base |
| Ca(OH)2 | Calcium hydroxide | 3 | Brønsted base | Strong base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CaSO4 | Calcium sulfate | 3 | Conjugate acid | Salt of strong base |
| Fe(OH)3 | Iron(III) hydroxide | 2 | Conjugate base | Weak base |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of iron(III) sulfate and calcium hydroxide
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | −408.6 | – | – | – |
per 1 mol of | −408.6 | – | – | – |
per 1 mol of | −136.2 | – | – | – |
per 1 mol of | −136.2 | – | – | – |
per 1 mol of | −204.3 | – | – | – |
Changes in standard condition (2)
- Reaction of iron(III) sulfate and calcium hydroxide
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | −382.0 | – | – | – |
per 1 mol of | −382.0 | – | – | – |
per 1 mol of | −127.3 | – | – | – |
per 1 mol of | −127.3 | – | – | – |
per 1 mol of | −191.0 | – | – | – |
Changes in standard condition (3)
- Reaction of iron(III) sulfate and calcium hydroxide
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | −368.6 | – | – | – |
per 1 mol of | −368.6 | – | – | – |
per 1 mol of | −122.9 | – | – | – |
per 1 mol of | −122.9 | – | – | – |
per 1 mol of | −184.3 | – | – | – |
Changes in aqueous solution (1)
- Reaction of iron(III) sulfate and calcium hydroxide◆
ΔrG −345.7 kJ/mol K 3.66 × 1060 pK −60.56
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | – | −345.7 | – | – |
per 1 mol of | – | −345.7 | – | – |
per 1 mol of | – | −115.2 | – | – |
per 1 mol of | – | −115.2 | – | – |
per 1 mol of | – | −172.8 | – | – |
Changes in aqueous solution (2)
- Reaction of iron(III) sulfate and calcium hydroxide◆
ΔrG −320.6 kJ/mol K 1.47 × 1056 pK −56.17
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | – | −320.6 | – | – |
per 1 mol of | – | −320.6 | – | – |
per 1 mol of | – | −106.9 | – | – |
per 1 mol of | – | −106.9 | – | – |
per 1 mol of | – | −160.3 | – | – |
Changes in aqueous solution (3)
- Reaction of iron(III) sulfate and calcium hydroxide◆
ΔrG −307.3 kJ/mol K 6.86 × 1053 pK −53.84
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | – | −307.3 | – | – |
per 1 mol of | – | −307.3 | – | – |
per 1 mol of | – | −102.4 | – | – |
per 1 mol of | – | −102.4 | – | – |
per 1 mol of | – | −153.7 | – | – |
Thermodynamic data of reactants
| Chemical formula | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
|---|---|---|---|---|
| Fe2(SO4)3 (cr) | -2581.5[1] | – | – | – |
| Fe2(SO4)3 (ai) | -2825.0[1] | -2242.8[1] | -571.5[1] | – |
| Ca(OH)2 (cr) | -986.09[1] | -898.49[1] | 83.39[1] | 87.49[1] |
| Ca(OH)2 (g) | -544[1] | – | – | – |
| Ca(OH)2 (ai) | -1002.82[1] | -868.07[1] | -74.5[1] | – |
| Ca(OH)2 (cr) 2 hydrate | -1218.4[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas
Thermodynamic data of products
| Chemical formula | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
|---|---|---|---|---|
| CaSO4 (cr) insoluble, anhydrite | -1434.11[1] | -1321.79[1] | 106.7[1] | 99.66[1] |
| CaSO4 (cr) soluble, α | -1425.24[1] | -1313.42[1] | 108.4[1] | 100.21[1] |
| CaSO4 (cr) soluble, β | -1420.80[1] | -1308.98[1] | 108.4[1] | 99.04[1] |
| CaSO4 (ai) | -1452.10[1] | -1298.10[1] | -33.1[1] | – |
| CaSO4 (cr) 0.5 hydrate macrocrystalline, α | -1576.74[1] | -1436.74[1] | 130.5[1] | 119.41[1] |
| CaSO4 (cr) 0.5 hydrate microcrystalline, β | -1574.65[1] | -1435.78[1] | 134.3[1] | 124.22[1] |
| CaSO4 (cr) 2 hydrate selenite | -2022.63[1] | -1797.28[1] | 194.1[1] | 186.02[1] |
| Fe(OH)3 (cr) precipitated | -823.0[1] | -696.5[1] | 106.7[1] | – |
| Fe(OH)3 (ao) | – | -659.3[1] | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution
References
List of references
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -2581.5 kJ · mol−1
- ^ ΔfH°, -2825.0 kJ · mol−1
- ^ ΔfG°, -2242.8 kJ · mol−1
- ^ S°, -571.5 J · K−1 · mol−1
- ^ ΔfH°, -986.09 kJ · mol−1
- ^ ΔfG°, -898.49 kJ · mol−1
- ^ S°, 83.39 J · K−1 · mol−1
- ^ Cp°, 87.49 J · K−1 · mol−1
- ^ ΔfH°, -544. kJ · mol−1
- ^ ΔfH°, -1002.82 kJ · mol−1
- ^ ΔfG°, -868.07 kJ · mol−1
- ^ S°, -74.5 J · K−1 · mol−1
- ^ ΔfH°, -1218.4 kJ · mol−1
- ^ ΔfH°, -1434.11 kJ · mol−1
- ^ ΔfG°, -1321.79 kJ · mol−1
- ^ S°, 106.7 J · K−1 · mol−1
- ^ Cp°, 99.66 J · K−1 · mol−1
- ^ ΔfH°, -1425.24 kJ · mol−1
- ^ ΔfG°, -1313.42 kJ · mol−1
- ^ S°, 108.4 J · K−1 · mol−1
- ^ Cp°, 100.21 J · K−1 · mol−1
- ^ ΔfH°, -1420.80 kJ · mol−1
- ^ ΔfG°, -1308.98 kJ · mol−1
- ^ S°, 108.4 J · K−1 · mol−1
- ^ Cp°, 99.04 J · K−1 · mol−1
- ^ ΔfH°, -1452.10 kJ · mol−1
- ^ ΔfG°, -1298.10 kJ · mol−1
- ^ S°, -33.1 J · K−1 · mol−1
- ^ ΔfH°, -1576.74 kJ · mol−1
- ^ ΔfG°, -1436.74 kJ · mol−1
- ^ S°, 130.5 J · K−1 · mol−1
- ^ Cp°, 119.41 J · K−1 · mol−1
- ^ ΔfH°, -1574.65 kJ · mol−1
- ^ ΔfG°, -1435.78 kJ · mol−1
- ^ S°, 134.3 J · K−1 · mol−1
- ^ Cp°, 124.22 J · K−1 · mol−1
- ^ ΔfH°, -2022.63 kJ · mol−1
- ^ ΔfG°, -1797.28 kJ · mol−1
- ^ S°, 194.1 J · K−1 · mol−1
- ^ Cp°, 186.02 J · K−1 · mol−1
- ^ ΔfH°, -823.0 kJ · mol−1
- ^ ΔfG°, -696.5 kJ · mol−1
- ^ S°, 106.7 J · K−1 · mol−1
- ^ ΔfG°, -659.3 kJ · mol−1